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Shib Sagar posted an Question
July 15, 2020 • 08:11 am 30 points
  • IIT JAM
  • Chemistry (CY)

We know that half and full filled e/c is most stable but when the condition is half filled vs full filled which one will get priority

we know that half and full filled E/C is most stable but when the condition is half filled vs full filled which one will get priority

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    Dinesh khalmaniya 1 Best Answer

    fully filled orbitals are more stable tha half filled because fully filled orbitals have morr exchange energy tha half filled. exchange energy can be calculated as

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    Dinesh khalmaniya 1

    check this video https://youtu.be/53iF1SkE-1M

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    Priyanshu kumar best-answer

    Similarly same case arises for p6 is more stable than p3...as in the case of p6 there is more exchange energy in comparison to p3...putting on exchange energy formula we get for p3 exchange energy = (3×2)/2K = 3K and for p6 it is 3K + 3K i.e 6 K.... so in this way you can compare it...

  • Suman Kumar

    Fully filled orbital are more stable as they have larger exchange energy.

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    Priyanshu kumar

    you know shib the half filled or completely filled orbitals are more stable then any other electronic configuration …….. this is because of a phenomenon known as exchange energy . Electrons are always in a state of motion , they are never still but according to the orbital diagrams it is shown that an electron occupies a particular set of quantum numbers and stays in a particular region ……. this is not true electrons always exchange their magentic quantum numbers , they stay in the same subshell but can travel to different orbitals For example for carbon if we consider , the electronic configuration is 1s2 2s2 2p2 so the two electrons of the 2p subshell are always in a state of motion and continiously change their places ( the exchange is not possible in case of s subshell because the electrons cannot change their spin) …….. that is why in half filled or completely filled orbitals the electrons get a larger area to change their positions as compared to any other electronic configuration and the stability increases as the electrons are in a state of dynamic equilibrium The greater the exchange energy , the more stable the atom is . The formula for calculating the exchange energy is Eex = (N(N-1))/2 *K , where N is the number of orbitals occupied by the electrons (not equal to magnetic quantum number , in some elements there is an exceptional electronic configuration such as cobalt, copper where the value of N is not equal to magnetic quantum number) and K is a specific constant in whose terms the exchange energy is expressed So for d5 type of electronic configuration , the value of Eex is (5*4)/2 * K Eex = 10 K And for d10 type of electronic configuration , the value of Eex is (5*4)/2 * K + (5*4)/2 * K (because the electrons with parellel spin can exchange theirpositions within themselves and the electrons with antiparellel spin can exchange their positions within themselves) Eex = 10 K + 10 K Eex = 20 K So the d10 type of electronic configuration is more stable than the d5 type of electronic configuration .

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